Final answer:
The balanced redox reaction occurring in the voltaic cell Al(s)|Al3+(aq)||Pb2+(aq)|Pb(s) is 2Al(s) + 3Pb2+(aq) → 2Al3+(aq) + 3Pb(s), involving the oxidation of aluminum and the reduction of lead.
Step-by-step explanation:
The question pertains to identifying the redox reaction that is taking place in a given voltaic cell represented by the cell notation Al(s)|Al3+(aq)||Pb2+(aq)|Pb(s). In a galvanic cell, two half-reactions occur: oxidation at the anode and reduction at the cathode. The aluminum (Al) acts as the anode where oxidation takes place, and lead (Pb) acts as the cathode where reduction occurs.
The half-reactions are as follows:
Oxidation (Anode): Al(s) → Al3+(aq) + 3e-
Reduction (Cathode): Pb2+(aq) + 2e- → Pb(s)
To balance the number of electrons transferred in both half-reactions, we multiply the aluminum half-reaction by 2 and the lead half-reaction by 3 and then add them together to get the balanced overall redox reaction:
2Al(s) + 3Pb2+(aq) → 2Al3+(aq) + 3Pb(s)
This balanced equation represents the chemical changes occurring as the galvanic cell operates, with aluminum metal being oxidized to aluminum ions while lead ions are reduced to lead metal.